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6 Cards in this Set
- Front
- Back
- 3rd side (hint)
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Why does disorder always increase? |
There are so many more ways things can be disorganized when occupy more space than organised. |
Think probability |
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Given 2 blocks of copper metal, one is 323 ℃ other 25 ℃, heat passes from hot to cold metal until they are in thermodynamic equilibrium.596 J of heat is passed from hot copper bar to cold. Calculate the entropy change of the 2 blocks. |
∆Shot = -596 J / 596 K = -1 J/K ∆Scold = 596 J / 298 K = 2 J/K
Total entropy change is -1 +2 = +1 J/K |
Use formula ∆S = qrev /T qrev is heat supplied to a reversible condition |
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What does spontaneous/feasible mean? |
Of natural process. A reaction may be spontaneous in thermodynamic sense, kinetics can still prevent from happening (activation barrier). |
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What makes chemical reaction go? |
∆G must be negative, entropy must increase. |
Think Gibbs energy |
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How is ∆G and ∆S correlated? |
University is made of a system and a surrounding, therefore ∆S universe = ∆Ssystem + ∆Ssurrounding And ∆S = q/T;
Under reversible condition ∆Suniverse = ∆Ssystem + qsurrounding /T
Any heat that has entered the surrounding must have left the system: ∆Suniverse = ∆Ssystem - qsystem/T
Under isobaric condition q = ∆H
∆Suniverse = ∆Ssystem - ∆Hsystem/TDevide both sides by -T and ∆G is defined as ∆G = ∆H - T∆S Devide both sides by -T and ∆G is defined as ∆G = ∆H - T∆S |
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What is ∆G in terms of chemical potential energy |
Difference in chemical potential between the products and reactants at the composition is the reaction mixture. |
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